US4192371A - Process for supplying thermal energy for an endothermic reaction from a source not available at the reaction site - Google Patents

Process for supplying thermal energy for an endothermic reaction from a source not available at the reaction site Download PDF

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US4192371A
US4192371A US05/824,308 US82430877A US4192371A US 4192371 A US4192371 A US 4192371A US 82430877 A US82430877 A US 82430877A US 4192371 A US4192371 A US 4192371A
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reaction
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Jean-Jacques Derouette
Jacques Dartoy
Jacques Fournier
Bernard Vollerin
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Bpifrance Financement SA
Battelle Memorial Institute Inc
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Agence National de Valorisation de la Recherche ANVAR
Battelle Memorial Institute Inc
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    • F—MECHANICAL ENGINEERING; LIGHTING; HEATING; WEAPONS; BLASTING
    • F28—HEAT EXCHANGE IN GENERAL
    • F28D—HEAT-EXCHANGE APPARATUS, NOT PROVIDED FOR IN ANOTHER SUBCLASS, IN WHICH THE HEAT-EXCHANGE MEDIA DO NOT COME INTO DIRECT CONTACT
    • F28D20/00—Heat storage plants or apparatus in general; Regenerative heat-exchange apparatus not covered by groups F28D17/00 or F28D19/00
    • F28D20/003—Heat storage plants or apparatus in general; Regenerative heat-exchange apparatus not covered by groups F28D17/00 or F28D19/00 using thermochemical reactions
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J19/00—Chemical, physical or physico-chemical processes in general; Their relevant apparatus
    • B01J19/08—Processes employing the direct application of electric or wave energy, or particle radiation; Apparatus therefor
    • B01J19/12—Processes employing the direct application of electric or wave energy, or particle radiation; Apparatus therefor employing electromagnetic waves
    • B01J19/122—Incoherent waves
    • B01J19/127—Sunlight; Visible light
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/06—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents
    • C01B3/061—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents by reaction of metal oxides with water
    • C01B3/063—Cyclic methods
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/06—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents
    • C01B3/068—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents the hydrogen being generated from the water as a result of a cyclus of reactions, not covered by groups C01B3/063 or C01B3/105
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/06—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents
    • C01B3/10—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents by reaction of water vapour with metals
    • C01B3/105—Cyclic methods
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/32—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air
    • C01B3/34—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents
    • C01B3/38—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide, air by reaction of hydrocarbons with gasifying agents using catalysts
    • F—MECHANICAL ENGINEERING; LIGHTING; HEATING; WEAPONS; BLASTING
    • F24—HEATING; RANGES; VENTILATING
    • F24S—SOLAR HEAT COLLECTORS; SOLAR HEAT SYSTEMS
    • F24S20/00—Solar heat collectors specially adapted for particular uses or environments
    • F24S20/20—Solar heat collectors for receiving concentrated solar energy, e.g. receivers for solar power plants
    • F—MECHANICAL ENGINEERING; LIGHTING; HEATING; WEAPONS; BLASTING
    • F24—HEATING; RANGES; VENTILATING
    • F24V—COLLECTION, PRODUCTION OR USE OF HEAT NOT OTHERWISE PROVIDED FOR
    • F24V30/00—Apparatus or devices using heat produced by exothermal chemical reactions other than combustion
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02B—CLIMATE CHANGE MITIGATION TECHNOLOGIES RELATED TO BUILDINGS, e.g. HOUSING, HOUSE APPLIANCES OR RELATED END-USER APPLICATIONS
    • Y02B10/00—Integration of renewable energy sources in buildings
    • Y02B10/20—Solar thermal
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E10/00—Energy generation through renewable energy sources
    • Y02E10/40—Solar thermal energy, e.g. solar towers
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/14—Thermal energy storage
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/30—Hydrogen technology
    • Y02E60/36—Hydrogen production from non-carbon containing sources, e.g. by water electrolysis
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E70/00—Other energy conversion or management systems reducing GHG emissions
    • Y02E70/30—Systems combining energy storage with energy generation of non-fossil origin

Definitions

  • Our present invention relates to a process for providing heat from a convenient source at a point of utilization at which that source is not readily available.
  • Thermal energy may be stored either directly or indirectly.
  • Direct storage utilizes the thermal capacity of various bodies, such as water, walls, rocks or soil, for example.
  • Indirect storage involving a conversion of sensible heat into latent heat or other forms of energy, makes use of such physical or chemical phenomena as melting, vaporization, solid/solid transformation or dissolution.
  • Direct-storage systems generally require large volumes of heat-storing materials, with attendant high costs and problems of space; in the absence of effective thermal insulation, which in many instances can be achieved only with difficulty or not at all, the occurrence of significant heat losses restricts this technique to short-term storage.
  • those based on conversion into chemical energy appear to be the most promising since they obviate the aforestated drawbacks and operate nearly without losses over prolonged periods.
  • the object of our present invention is to provide an efficient process for the chemical storage of thermal energy from an intermittent or localized source, such as the sun, for utilization at a point where such energy would otherwise be unavailable.
  • the thermal energy released at the recombination site can be used for a variety of purposes, including space heating.
  • a particularly advantageous use is for the promotion of an endothermic reaction which may or may not involve the component or components of the starting compound transferred to the recombination site.
  • the transferred component may be a metal or a lower oxide reacting exothermically with atmospheric oxygen or with some other locally available oxidant such as water; in the latter instance, the reaction liberates hydrogen which can then be used for industrial purposes.
  • Other locally available compounds, especially organic substances can be decomposed by the released thermal energy to produce, for instance, a synthesis gas.
  • Energy sources other than the sun which may be classified as limitedly available within the context of our invention, include geothermal springs whose heat output can thus be utilized at remote locations; similar considerations apply to industrial generators of waste heat, such as nuclear reactors, which exist only in a few widely separated places. They further include municipal utilities and the like supplying power at lower rates at certain times (usually at night) so that storage of their energy for use at other times is economically desirable.
  • a quantity of the recycled substances i.e. the component or components to be transferred to the recombination site in step (b) and the reconstituted starting compound to be retransferred to the dissociation site in step (d), to bridge any intervals during which the primary source of energy is absent, inoperative or more expensive.
  • the length of storage may range from a few minutes, as in the case of atmospheric disturbances or a solar eclipse, to a period of many months, e.g. in situations where sufficient sunlight is only seasonally available.
  • the endothermically dissociable substances capable of being utilized in a process according to our invention may be generally designated AX, where A represents a component or group of components to be recycled and X is another component or group of components which is available at the recombination site without recycling.
  • AX represents a component or group of components to be recycled
  • X is another component or group of components which is available at the recombination site without recycling.
  • the nonrecycled component or group of components X may be available in the form X m Y n , i.e. as a constituent of a different compound.
  • the recombination process restoring the original compound AX is of the form
  • components A and X are in different states of aggregation upon dissociation from each other, e.g. solid or liquid in the case of A and gaseous in the case of X, to simplify their separation.
  • the choice of substances to be used as starting compounds must also take into account a number of other factors, such as density of the material, stability of the reaction products, operating temperatures, reactivity of the component, corrosion, toxicity and cost; although theoretically there could be an infinite number of recyclings, some losses will occur in practice so that either the starting compound or its recycled component or components will have to be replenished from time to time.
  • the aforedescribed general reactions (101) and (102) can be divided into three families.
  • the first family encompasses systems using atmospheric oxygen as a reactant. These reactions will then have the form
  • R being a metal or metalloid and p being an integer greater than zero.
  • the dissociation process corresponds in this instance to a reduction of the starting compound from a higher oxide to a lower one, or possibly to its elemental state.
  • RO p /RO p-1 are the following:
  • Some of these reactions are promoted by luminous radiation, i.e. by solar photons accompanying the thermal energy derived from the sun.
  • the second family uses hydrates or hydroxides as starting compounds.
  • This family may be subdivided into two classes, one of them involving no separation of hydrogen and oxygen whereas the other utilizes water as a reactant.
  • the reactions relating to systems of the first class of this family can be represented by
  • A is a hydratable substance and n represents the number of water molecules contained in the hydrate employed.
  • reaction (402') may or may not take place within the system.
  • the starting compound is of the form MXO 2 where M is a metal (e.g. calcium, magnesium or manganese) and X is a multivalent nonmetal, preferably carbon or sulfur. If the starting compound is a carbonate, the reactions are
  • Lithium carbonate and barium or zinc sulfate could also be used.
  • FIG. 1 is a block diagram illustrating the process according to our invention
  • FIGS. 2 and 3 are graphs showing the dissociation and recombination of a representative oxide and a representative carbonate, respectively, in a system according to our invention
  • FIGS. 4 and 5 are diagrams similar to FIG. 1, illustrating certain modifications
  • FIG. 6 is a diagrammatic view of an installation used for carrying out our process, shown in vertical section;
  • FIG. 7 is a diagrammatic view of another such installation, shown in elevation.
  • FIG. 8 is a view similar to FIG. 7, illustrating a further modification.
  • FIG. 9 is a block diagram representing a more complex system.
  • a recycling system 3 includes a dissociation site in the form of a reactor 6, receiving solar energy 4, and a recombination site in the form of a reactor 9, delivering heat 5 to the area 1.
  • Reactor 6 has an entrance 7 for a compound AX and an exit 8 where its components A and X are separately discharged.
  • Component A is delivered to an entrance 10 of reactor 9 via a conduit 12 including a reservoir 13 for the interim storage of that component.
  • a compound X m Y n also fed to entrance 10 is a compound X m Y n reacting exothermally with component A, complementing the latter to a replica of the starting compound AX while leaving the site 9 at an exit 11 in the form X m-1 Y n .
  • the component X can also be recycled from reactor 6 via a conduit 12a after interim storage in a reservoir 13a; in that case, of course, the product X m-1 Y n is nonexistent.
  • the reconstituted compound AX is fed back to entrance 7 of reactor 6 via a conduit 14 containing a reservoir 15 for interim storage.
  • solar heat 4 is converted in reactor 6 into chemical energy and is then reconverted into free thermal energy 5 in reactor 9.
  • the carrier component A and the reconstituted starting compound AX can be recycled indefinitely, with infeed of additional material A via an inlet 13b of reservoir 13 to compensate for unavoidable losses.
  • the storage capacity of the several reservoirs should be sufficient to account for expected fluctuations in supply and demand.
  • reservoirs 13 and 15 are thermally insulated, surplus energy available in either reactor 6, 9 may be preserved at least for short periods in the form of sensible heat supplementing the chemically stored energy.
  • FIG. 2 we have plotted enthalpy ⁇ H (in kcal/mole) against temperature T (in degrees K) for the process given by reactions (201) and (202), with CuO as the starting material.
  • the enthalpy increases slowly up to a temperature of about 1150° K. and then jumps suddenly from about 20 to 50 kcal/mole with the release of O 2 and reduction of the starting compound to Cu 2 O.
  • the latter compound is allowed to cool to about 400° K. and then exothermally reacts with oxygen supplied at the recombination site to release the chemically stored heat while being reconverted to CuO.
  • the change in heat content, ⁇ H amounts to +31.5 kcal/mole on dissociation and to -34.5 kcal/mole on recombination.
  • FIG. 3 represents a similar graph for reactions (501) and (502), with CaCO 3 used as the starting compound.
  • dissociation occurs at about 1000° K., with ⁇ H ⁇ +43 kcal/mole, whereas recombination takes place at 600° K., with ⁇ H ⁇ -38 kcal/mole.
  • a suitable additive such as carbon
  • thermal reduction of ZnO to Zn calls for temperatures above the sublimation point of 1800° C., yet with the help of a carbonaceous substance such as pyrolytic charcoal, for example, the temperature can be lowered to about 1000° C.
  • the charcoal acting as a reducing agent, initially produces carbon monoxide which further reacts with the zinc oxide; the process in the dissociation reactor 6, FIG. 4, is then given by
  • the recombination site 9 may be merged with the point of utilization 1 in a common enclosure 18 in which the exothermic reaction A+X ⁇ AX promotes an endothermic reaction X m Y n ⁇ X m-1 Y n where X m-1 Y n is a desired industrial product; the endothermic reaction within enclosure 18 will generally proceed in a temperature range substantially lower--e.g. by about 100° to 200° C.--than the temperature range of the exothermic reaction.
  • the compound X m Y n to be decomposed may be a locally abundant substance, such as water.
  • the processes involved may be
  • the thermal decomposition of the zinc oxide at the dissociation site 6 requires a temperature on the order of 2200° K., or more than 1800° C., as indicated above whereas the decomposition of water in the presence of zinc vapor occurs at less than 900° C.
  • the aforedescribed expedient of lowering the dissociation temperature of ZnO by the admixture of elemental carbon can be used also in this instance.
  • FIG. 6 illustrates an apparatus for carrying out the reactions (801) and (802) without the use of a special reducing agent.
  • the apparatus comprises a chamber 21, corresponding to the reactor 18 of FIG. 5, in which water is to be decomposed to release hydrogen which is discharged via an outlet 24 for further utilization.
  • Another chamber 22, corresponding to reactor 6 of FIG. 6, serves for the dissociation of zinc oxide into metallic zinc and oxygen, in the presence of highly concentrated solar radiation 4 entering that chamber through a window 28.
  • the sun's rays may be focused upon a heliostatic reflector which keeps them trained upon the window 28.
  • Compartment 29 plays the part of a reservoir such as the store 13 shown in FIG. 5.
  • liquefied zinc present in compartment 29 enters several parallel conduits 27 (only one shown) which are in heat-exchanging relationship with chamber 22 whereby the zinc in these conduits is revaporized and rises into chamber 21.
  • Water from a nonillustrated source is vaporized, either by waste heat from chamber 22 or by other heating means not shown, as it passes into the same chamber 21 via a channel 23.
  • the steam and the zinc gases interact within that chamber, at a temperature below 900° C., to form pulverent zinc oxide and gaseous hydrogen, the zinc ozide then descending by gravity along a partition 25 between chambers 21 and 22 into an inlet 26 of the latter chamber where it forms a pile exposed to the incoming solar radiation for a repetition of the cycle.
  • the duct 24 includes a water trap 30 designed to condense water vapors entrained by the hydrogen gas leaving the chamber 21.
  • the store 15 of FIG. 5 is here represented by the lower part of chamber 22 containing the mass of zinc oxide whose mean temperature is now well above the boiling point of zinc and which is traversed by the conduits 27.
  • the system of FIG. 6 may have an ancillary inlet, not shown, for the introduction of zinc or zinc oxide to compensate for losses incurred in operation.
  • the system of FIG. 5 can also be utilized, for example, to produce a synthesis gas of the general formula
  • Reaction (901) takes place in chamber 6 whereas the others occur in chamber 18.
  • reaction (902) is the exothermic recombination process
  • reaction (903) is of pyrolytic nature
  • endothermic reactions (904)-(906) are a series of gasification steps which convert the free carbon of reaction (903) and a corresponding amount of water into the various constituents of a synthesis gas.
  • a rotary solar furnace 41 heated to high temperatures by incident radiation 4, has an inlet 42 and two exits 43 and 44.
  • a gasifying reactor 46 of the fluidized-bed type including a cracking catalyst such as Raney nickel, has inlets 47-49 and outlets 50-52.
  • a fluidized-bed separator 54 has an inlet 55 communicating with reactor outlet 51, an outlet 57 communicating with reactor inlet 49, an air inlet 56, an air outlet 53 and a further outlet 58.
  • a first store 59 is inserted between furnace outlet 43 and reactor inlet 47 whereas a second store 60 lies between reactor outlet 50 and furnace inlet 42.
  • a supplemental inlet 61 merges with outlet 50 at the entrance of store 60.
  • the thermally dissociable starting material is a mixture of magnesium oxide and calcium carbonate (derived from dolomite) stored in reservoir 60 and loaded via inlet 42 into solar furnace 41.
  • the presence of magnesium oxide lowers the dissociation temperature of the calcium carbonate in furnace 41 to a level on the order of 900°-1000° C.
  • the endothermic dissociation of MgO.CaCO 3 in the solar furnace releases carbon dioxide which escapes into the atmosphere at outlet 44.
  • the reduced mixture MgO.CaO is temporarily stored in reservoir 59 whence it enters, at the requisite rate, the reactor 46 for recombination with CO 2 admitted into that reactor through its inlet 48; this gas could, of course, be the same that leaves the furnace 41 at exit 44. Lignite and water vapor are introduced into the reactor by way of its inlet 49.
  • the reconstitution of the starting material MgO.CaCO 3 within reactor 46 converts the lignite and water vapor into a raw synthesis gas pursuant to reactions (903)-(906) which is available at outlet 52, leaving a residue of charcoal and ashes exiting from the reactor at 51 and entering the separator 54 at 55.
  • Part of the synthesis gas may be recycled to the reactor inlet 48, as indicated in dotted lines, to lower the partial water-vapor pressure therein.
  • the charcoal is returned from the separator 54 to the reactor 46 via connection 57/49 while the ashes are discharged at outlet 58.
  • the recycling of the charcoal converts the residual carbon into constituents of the synthesis gas, as discussed above with reference to reactions (904)-(906), to insure a maximum yield for a given quantity of raw material (lignite).
  • a natural mixture of magnesium and calcium carbonates can be introduced into the store 60 by way of inlet 61 for subsequent transformation into the dissociation product MgO.CaO.
  • Reaction (1001), taking place in chamber 6, is again endothermic, as is reaction (1004) proceeding from left to right within chamber 18 until terminated by a state of equilibrium; with higher temperatures, the latter reaction shifts further toward the right with generation of more elemental hydrogen.
  • the recombination process (1002) is strongly exothermic while reactions (1003) and (1005) are weakly so.
  • Reactions (1003)-(1005) are again promoted by the presence of a cracking catalyst, such as Raney nickel, on a refractory carrier.
  • the dissociation temperature in reactor 6 is on the order of 1200° C. while the operating temperature within reactor 18 is at a level of approximately 900°-1000° C.
  • FIG. 8 shows an installation designed to carry out the process just described.
  • a rotary solar furnace 62 again irradiated with solar energy 4 in the aforementioned manner, has an inlet 63 for lithium carbonate and two outlets 64, 65 for the discharge of lithium oxide and carbon dioxide, respectively.
  • Outlet 64 communicates via a store 73 with an inlet 67 of a fluidized-bed reactor 66 provided with two further inlets 68 and 69; the former receives CO 2 (possibly from furnace outlet 65, as shown) and water vapor, while the latter serves for the introduction of a light hydrocarbon such as naphtha.
  • the bed 77 of reactor 66 contains a catalytic charge such as nickel-coated ceramic pellets.
  • An outlet 72 serves for the discharge of raw synthesis gas, part of which may be recycled to inlet 68 to lower the partial water-vapor pressure in the reactor, while another outlet 70 delivers the reconstituted lithium carbonate via a store 74 to inlet 63 of furnace 62.
  • An ancillary inlet 75, merging with outlet 70, is again provided for replenishing purposes; instead of introducing supplemental Li 2 CO 3 into the store 74 through this inlet 75, it would also be possible to load the store 73 with additional LiO 2 via an inlet not shown.
  • the operating temperature in furnace 62 required for the dissociation of Li 2 CO 3 according to reaction (1001), is about 1200° C. while that in reactor 66 is a few hundreds of degrees lower, as noted above.
  • FIG. 9 we have schematically illustrated an installation for the production of hydrogen by a process according to our invention which uses a primary and a secondary cycle for the decomposition of water.
  • the primary cycles involves dissociation of barium sulfate in a main reactor 81, with interim storage of the resulting barium sulfide in a reservoir 101 connected to an outlet 84 of that reactor.
  • the stored barium sulfide is fed to an inlet 88 of another reactor 86 receiving water (or steam) via another inlet 87.
  • the interaction of these components in reactor 86 yields hydrogen, removed at an outlet 90, and barium sulfate exiting at another outlet 89 to a reservoir 102 for interim storage prior to introduction into reactor 81 by an inlet 82 thereof.
  • Sulfur dioxide another product of dissociation, leaves the reactor 81 at an outlet 85 and, after interim storage in a reservoir 106, is supplied to an inlet 98 of a reactor 96 to participate in the secondary cycle in which the starting material is zinc sulfate, dissociated in a reactor 91 to zinc oxide, sulfur dioxide and oxygen.
  • the oxygen is discharged into the atmosphere at an outlet 93 while the other reaction products are delivered by way of respective outlets 94 and 95 to a store 103 of the zinc oxide and a store 104 for the sulfur dioxide; these two compounds are then fed into reactor 96 via inlets 97 and 98, respectively, to reconstitute the original zinc sulfate which leaves the reactor at an outlet 100 and is recycled to reactor 91 via a store 105 and an outlet 92.
  • the reaction in vessel 96 also yields free sulfur which is admitted to reactor 81 through an inlet 83 thereof via a store 107 in order to assist in the reduction of the barium sulfate.
  • the two reactors 81 and 91 are irradiated with solar energy 4 as required for the endothermic processes taking place therein.

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US05/824,308 1976-08-13 1977-08-12 Process for supplying thermal energy for an endothermic reaction from a source not available at the reaction site Expired - Lifetime US4192371A (en)

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CH10312/76 1976-08-13
CH1031276A CH617503A5 (enrdf_load_stackoverflow) 1976-08-13 1976-08-13

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US4279227A (en) * 1972-10-27 1981-07-21 Skala Stephen F Heat storage in by-products of an intermittent process
US4309980A (en) * 1980-03-07 1982-01-12 Thermal Energy Storage, Inc. Closed vaporization heat transfer system
US4332139A (en) * 1978-12-27 1982-06-01 The Director-General Of The Agency Of Industrial Science And Technology Method for storage and recovery of thermal energy
WO1982002590A1 (en) * 1981-01-19 1982-08-05 Technologies Corp United Self-driven chemical heat pipe
US4436539A (en) 1981-10-06 1984-03-13 Technion Research And Development Foundation Ltd. Method and apparatus for air-conditioning by means of a hydrogen heat pump
WO1985002010A1 (en) * 1983-10-28 1985-05-09 Robert Floyd Butler Process for the reversible transfer of thermal energy and heat transfer system useful therein
US5661977A (en) * 1995-06-07 1997-09-02 Shnell; James H. System for geothermal production of electricity
WO1996041104A3 (en) * 1995-06-07 1998-02-26 James H Shnell System for geothermal production of electricity
US20080099404A1 (en) * 2006-11-01 2008-05-01 Rimkus Consulting Group, Inc. Corporation Of Texas Process and apparatus for treating industrial effluent water with activated media
US20100163231A1 (en) * 2008-12-31 2010-07-01 Chevron U.S.A. Inc. Method and system for producing hydrocarbons from a hydrate reservoir using available waste heat
US20120266863A1 (en) * 2011-04-20 2012-10-25 Surendra Saxena Solar-Hydrogen Hybrid Storage System for Naval and Other Uses
EP2520361A1 (en) * 2011-05-06 2012-11-07 ETH Zurich Method for thermochemically reacting a particulate material and apparatus for conducting said method
US20140298822A1 (en) * 2013-04-03 2014-10-09 Alliance For Sustainable Energy, Llc Chemical Looping Fluidized-Bed Concentrating Solar Power System and Method
US20150253039A1 (en) * 2012-10-16 2015-09-10 Luke Erickson Coupled chemical-thermal solar power system and method
US20220379280A1 (en) * 2020-02-20 2022-12-01 Doosan Lentjes Gmbh Method for operating a fluidized bed apparatus and fluidized bed apparatus
US11740031B1 (en) * 2022-03-04 2023-08-29 Battelle Savannah River Alliance, Llc High temperature thermochemical energy storage materials

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DE2905206A1 (de) * 1979-02-12 1980-08-21 Interatom Anlage zur thermochemischen wasserspaltung mit sonnenenergie
DE3337078A1 (de) * 1983-10-12 1985-05-02 M.A.N. Maschinenfabrik Augsburg-Nürnberg AG, 8000 München Verfahren und vorrichtung zum herstellen von synthesegas
ES2574352B1 (es) * 2014-12-15 2017-03-28 Abengoa Solar New Technologies, S.A. Planta de potencia con almacenamiento termoquímico basado en un ciclo de reacciones y su método de funcionamiento

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US3075361A (en) * 1957-11-08 1963-01-29 Jr John E Lindberg Method and apparatus for transferring heat
US3958625A (en) * 1974-07-01 1976-05-25 General Electric Company Transport of heat as chemical energy
US3967676A (en) * 1974-07-01 1976-07-06 General Electric Company Transport of heat as chemical energy
US3972183A (en) * 1975-04-17 1976-08-03 Chubb Talbot A Gas dissociation thermal power system
US4044819A (en) * 1976-02-12 1977-08-30 The United States Of America As Represented By The United States Energy Research And Development Administration Hydride heat pump

Cited By (28)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4279227A (en) * 1972-10-27 1981-07-21 Skala Stephen F Heat storage in by-products of an intermittent process
US4332139A (en) * 1978-12-27 1982-06-01 The Director-General Of The Agency Of Industrial Science And Technology Method for storage and recovery of thermal energy
US4309980A (en) * 1980-03-07 1982-01-12 Thermal Energy Storage, Inc. Closed vaporization heat transfer system
WO1982002590A1 (en) * 1981-01-19 1982-08-05 Technologies Corp United Self-driven chemical heat pipe
US4346752A (en) * 1981-01-19 1982-08-31 United Technologies Corporation Self-driven chemical heat pipe
US4436539A (en) 1981-10-06 1984-03-13 Technion Research And Development Foundation Ltd. Method and apparatus for air-conditioning by means of a hydrogen heat pump
WO1985002010A1 (en) * 1983-10-28 1985-05-09 Robert Floyd Butler Process for the reversible transfer of thermal energy and heat transfer system useful therein
US5661977A (en) * 1995-06-07 1997-09-02 Shnell; James H. System for geothermal production of electricity
US5697218A (en) * 1995-06-07 1997-12-16 Shnell; James H. System for geothermal production of electricity
WO1996041104A3 (en) * 1995-06-07 1998-02-26 James H Shnell System for geothermal production of electricity
AU700526B2 (en) * 1995-06-07 1999-01-07 James H. Shnell System for geothermal production of electricity
US5911684A (en) * 1995-06-07 1999-06-15 Shnell; James H. System for geothermal production of electricity
US7491336B2 (en) 2006-11-01 2009-02-17 Rimkus Consulting Group, Inc. Process for treating industrial effluent water with activated media
WO2008057358A3 (en) * 2006-11-01 2008-08-28 Rimkus Consulting Group Inc Process and apparatus for treating industrial effluent water with activated media
US20080099404A1 (en) * 2006-11-01 2008-05-01 Rimkus Consulting Group, Inc. Corporation Of Texas Process and apparatus for treating industrial effluent water with activated media
US7879245B2 (en) 2006-11-01 2011-02-01 Markham Gary W Process for treating industrial effluent water with activtated media
US20100163231A1 (en) * 2008-12-31 2010-07-01 Chevron U.S.A. Inc. Method and system for producing hydrocarbons from a hydrate reservoir using available waste heat
US8201626B2 (en) * 2008-12-31 2012-06-19 Chevron U.S.A. Inc. Method and system for producing hydrocarbons from a hydrate reservoir using available waste heat
US20120266863A1 (en) * 2011-04-20 2012-10-25 Surendra Saxena Solar-Hydrogen Hybrid Storage System for Naval and Other Uses
EP2520361A1 (en) * 2011-05-06 2012-11-07 ETH Zurich Method for thermochemically reacting a particulate material and apparatus for conducting said method
WO2012152413A1 (en) * 2011-05-06 2012-11-15 Eth Zurich Method for thermochemically reacting a particulate material and apparatus for conducting said method
US20150253039A1 (en) * 2012-10-16 2015-09-10 Luke Erickson Coupled chemical-thermal solar power system and method
US20140298822A1 (en) * 2013-04-03 2014-10-09 Alliance For Sustainable Energy, Llc Chemical Looping Fluidized-Bed Concentrating Solar Power System and Method
US9702348B2 (en) * 2013-04-03 2017-07-11 Alliance For Sustainable Energy, Llc Chemical looping fluidized-bed concentrating solar power system and method
US20220379280A1 (en) * 2020-02-20 2022-12-01 Doosan Lentjes Gmbh Method for operating a fluidized bed apparatus and fluidized bed apparatus
US11779895B2 (en) * 2020-02-20 2023-10-10 Doosan Lentjes Gmbh Method for operating a fluidized bed apparatus and fluidized bed apparatus
US11740031B1 (en) * 2022-03-04 2023-08-29 Battelle Savannah River Alliance, Llc High temperature thermochemical energy storage materials
US20230280104A1 (en) * 2022-03-04 2023-09-07 Battelle Savannah River Alliance, Llc High temperature thermochemical energy storage materials

Also Published As

Publication number Publication date
CH617503A5 (enrdf_load_stackoverflow) 1980-05-30
FR2361148B1 (enrdf_load_stackoverflow) 1982-01-22
IT1083945B (it) 1985-05-25
FR2361148A1 (fr) 1978-03-10

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